52.05 liters of hydrogen gas are produced at 298 K and 0.940 atm if 4.00 moles of hydrochloric acid react with an excess of magnesium metal.
The ideal gas law states that the pressure of a gas is directly proportional to the volume and temperature of the gas.
It is expressed as
PV = nRT
where,
P is pressure
V is volume in liters
n is number of moles of gas
R is Ideal gas constant
T is Temperature in kelvin
The balanced chemical equation is the equation in which the number of atoms on the reactant side is equal to the number of atoms on the product side in an equation.
Now first we have to write the balanced chemical equation
Mg + 2HCl → MgCl₂ + H₂
Here we can se that 2 mole of hydrochloric acid produces 1 mole of hydrogen gas.
So 4 moles of hydrochloric gas will give [tex]\frac{1}{2} \times 4[/tex] moles of hydrogen gas that is 2 moles of hydrogen gas.
Now put the values in above equation, we get
PV = nRT
0.940 atm × V = 2 × 0.0821 L atm / K mol × 298
V = [tex]\frac{2 \times 0.0821\ \text{L atm / K mol} \times 298}{0.940\ \text{atm}}[/tex]
V = 52.05 liter
Thus from the above conclusion we can say that 52.05 liters of hydrogen gas are produced at 298 K and 0.940 atm if 4.00 moles of hydrochloric acid react with an excess of magnesium metal.
Learn more about the Ideal gas law here: https://brainly.com/question/25290815
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